Refer to the nomenclature flowchart (Figure 3.11) to name each compound. c. CoSO4

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Identify the cation and the anion in the compound CoSO₄.

Recognize that Co represents cobalt, which is a transition metal and can have multiple oxidation states.

Determine the charge of the sulfate ion (SO₄²⁻), which is a polyatomic ion with a -2 charge.

Since the compound is neutral, the charge of the cobalt ion must balance the charge of the sulfate ion. Therefore, the cobalt ion must have a +2 charge.

Name the compound by stating the name of the cation followed by the name of the anion. Use Roman numerals to indicate the oxidation state of the cobalt ion: Cobalt(II) sulfate.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionic Compounds

Ionic compounds are formed from the electrostatic attraction between positively charged cations and negatively charged anions. In the case of CoSO4, cobalt (Co) acts as the cation, while the sulfate ion (SO4) serves as the anion. Understanding the nature of ionic bonds is essential for correctly naming and identifying these compounds.

Nomenclature of Transition Metals

Transition metals can exhibit multiple oxidation states, which affects how they are named in compounds. The oxidation state of the metal is indicated by a Roman numeral in parentheses following the metal's name. For CoSO4, cobalt typically has a +2 oxidation state, leading to the name cobalt(II) sulfate.

Polyatomic Ions

Polyatomic ions are ions composed of two or more atoms covalently bonded together, which carry a net charge. The sulfate ion (SO4) is a common polyatomic ion with a -2 charge. Recognizing polyatomic ions and their charges is crucial for correctly naming compounds that include them, such as CoSO4.

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